In the Haber process, ammonia is synthesized from N2 and H2. Given the reaction N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) and ΔG° at 298 K is –33.3 kJ/mol, what is the value of ΔG at 298 K for a reaction mixture with partial pressures of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3?

Given the reaction Cl2(g) + 2NO(g) → 2NOCl(g), if the standard Gibbs free energy change (ΔG°) for the reaction is negative, what can be concluded about the reaction at standard conditions?

Determine the minimum pressure of N₂ required to keep the reaction N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) spontaneous at 298 K, given ΔG°rxn = -33.3 kJ/mol, P H₂ = 1.00 x 10⁻² atm, and P NH₃ = 1.00 atm.

Estimate the value of the equilibrium constant at 660 K for the reaction 2NO2(g) ⇌ N2O4(g) given that ΔG°f for BrCl(g) is -1.0 kJ/mol and the standard molar entropy, S°, for BrCl(g) is 240.0 J/mol⋅K. Assume ΔH°f for N2O4(g) is -9.2 kJ/mol and ΔH°f for NO2(g) is 33.2 kJ/mol.

For the reaction A (g) ⇌ 2 B (g), K = 14.7 at 298 K, what is the value of the reaction quotient Q at 298 K when ΔG = 19.6 kJ/mol?

For the reaction A(g) ⇌ B(g) with ΔG° = 31.5 kJ at 298K, if the initial concentration of A is 0.100 M, what is the equilibrium concentration of B?

Using standard free energy of formation values, calculate the equilibrium constant Kp for the reaction Cl2(g) + 2NO(g) ↔ 2NOCl(g) at 298 K. Given that the standard free energy change (ΔG°) for the reaction is -33.0 kJ/mol, what is the value of Kp?

What is the relationship between the equilibrium constant (Kₚ), the reaction quotient (Qₚ), and the standard equilibrium constant (K₀) for a reaction involving gases?

When adjusted for any changes in ΔH and ΔS with temperature, the standard free energy change ΔG°T at 2400 K is equal to 1.22×10^5 J/mol. Calculate the equilibrium constant (K) at 2400 K.